Multiple Choice
What is the value (in V) of E°cell for the following reaction? Zn2+ (aq) + Pb (s) ⇌ Zn (s) + Pb2+ (aq)
20. Electrochemistry
Standard Reduction Potentials
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Identify the species that is being oxidized in the following balanced reaction.
3 Pb2+ (aq) + 2 Cr (s) → 3 Pb (s) + 2 Cr3+ (aq)
A
Pb2+
B
Cr3+
C
Pb
D
Cr
Verified step by step guidance1
Identify the oxidation states of each element in the reactants and products. For Pb2+ (aq), the oxidation state is +2. For Cr (s), the oxidation state is 0. For Pb (s), the oxidation state is 0. For Cr3+ (aq), the oxidation state is +3.
Determine the change in oxidation states for each element. Pb2+ changes from +2 to 0, indicating a reduction. Cr changes from 0 to +3, indicating an oxidation.
Recognize that oxidation involves an increase in oxidation state, while reduction involves a decrease in oxidation state.
Identify the species that undergoes an increase in oxidation state. In this reaction, Cr goes from an oxidation state of 0 to +3.
Conclude that the species being oxidized is Cr, as it experiences an increase in oxidation state from 0 to +3.
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